Textbook Question
Use hybrid orbitals to draw the following molecules.
(d)
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1. A Review of General Chemistry
Hybridization
3:10 minutesProblem 51i,j
Textbook Question
What is the hybridization of all the atoms (other than hydrogen) in each of the following?
What are the bond angles around each atom?
i. H3O+
j. H2C═O
Verified step by step guidance1
Step 1: For H₃O⁺ (hydronium ion), identify the central atom and its bonding. The central atom is oxygen, which is bonded to three hydrogen atoms and has one lone pair of electrons. This gives a total of four regions of electron density around the oxygen atom.
Step 2: Determine the hybridization of the oxygen atom in H₃O⁺. Since there are four regions of electron density (three bonds and one lone pair), the hybridization of oxygen is sp³. Use the formula: hybridization = number of sigma bonds + number of lone pairs.
Step 3: Predict the bond angles around the oxygen atom in H₃O⁺. The ideal bond angle for sp³ hybridization is 109.5°, but due to the lone pair repulsion, the bond angles will be slightly less than 109.5°.
Step 4: For H₂C═O (formaldehyde), identify the central atom and its bonding. The central atom is carbon, which is double-bonded to oxygen and single-bonded to two hydrogen atoms. This gives a total of three regions of electron density around the carbon atom.
Step 5: Determine the hybridization and bond angles for the carbon atom in H₂C═O. With three regions of electron density, the carbon atom is sp² hybridized. The bond angles around the carbon atom are approximately 120°, which is characteristic of sp² hybridization and a trigonal planar geometry.
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Video duration:
3mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate the bonding requirements of an atom. In organic chemistry, it helps explain the geometry and bonding properties of molecules. For example, sp3 hybridization involves one s and three p orbitals, resulting in a tetrahedral shape, while sp2 involves one s and two p orbitals, leading to a trigonal planar arrangement.
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Bond Angles
Bond angles are the angles formed between adjacent bonds in a molecule, which are determined by the hybridization of the central atom. These angles reflect the spatial arrangement of the electron pairs around the atom. For instance, in sp3 hybridized molecules, the bond angles are approximately 109.5 degrees, while in sp2 hybridized molecules, they are about 120 degrees.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonding pairs and lone pairs of electrons around the central atom, which dictate the shape of the molecule. Understanding molecular geometry is crucial for predicting the physical and chemical properties of compounds, such as polarity and reactivity.
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